Question

Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10−2M . At equilibrium, [Cl2]= 1.3×10−2M . Calculate the value of the equilibrium constant (Kc).

Answer 1

The value of equilibrium constant is equal to the quotient of the products raised to its stoichiometric coefficient over the reaction's reactants raised to its respective stoichiometric coeff. The equation is Kc=[SO2][Cl2]/[SO2Cl2]= [1.3*10^-2][1.3*10^-2]/[2.2*10^-2-1.3*10^-2]=0.0188. The final answer is Kc=0.0188.